Textbook Problem

Consider a cell based on the following half-reactions:

a. Draw this cell under standard conditions, labeling the anode, the cathode, the direction of electron flow, and the concentrations, as appropriate.

b. When enough NaCl(s) is added to the compartment containing gold to make the [Cl⁻] = 0.10 M, the cell potential is observed to be 0.31 V. Assume that Au³⁺ is  reduced and assume that the reaction in the compartment containing gold is

${\text{Au}}^{3+}\left(aq\right)+4{\text{Cl}}^{-}\left(aq\right)\rightleftharpoons {\text{AuCl}}_4{}^{-}\left(aq\right)$

Calculate the value of K for this reaction at 25°C.